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April 16, 2014

Search: Chemistry, pH, Buffers

Number of results: 102,718

chemistry
Buffer capacity can be defined in a variety of ways; the one I use is, "the mols of strong acid or strong base that can be added to 1 L of a buffer that will change the pH by 1 unit. You look at your graph and read the beginning pH and mols (say acid) then find the pH that is ...
Saturday, April 14, 2012 at 11:07am by DrBob222

Chemistry
Buffers are commonly at a neutral pH of 7; this is wrong. Buffers are usually equal to the pKa or pKb of the acid and its conjugate base, or the base and its conjugate acid. You are right: they do counter act the addition of an acid by by making more of its conjugate base, or ...
Thursday, March 14, 2013 at 2:20am by Devron

chemistry
How do basic and acidic buffers resist pH ?
Thursday, September 23, 2010 at 10:54pm by CHELsea

chemistry
Buffers resist a change in pH. The DO change pH, however. They do not prevent a change from taking place.
Tuesday, April 8, 2008 at 9:43pm by DrBob222

chemistry
One thing to learn quickly in buffers is that when bae = acid(as in this case) is that pH = pKa. You know Ka so -log Ka = pKa = pH
Wednesday, December 5, 2012 at 11:29am by DrBob222

chemistry lab
Could someone help me with this? i am tired of it. here is my data from lab: Buffer1: HPO4- weight 3.412g; original pH Buffer 2: HEPES wt: 1.090g original pH 10.08 buffer1: pH of 0.1M: 7.5; pH of 0.01: 7.72; pH of 0.001M: 7.87 buffer2: PH of 0.1M: 7.5 ph of 0.01 M: 7.42 pH of ...
Friday, February 1, 2008 at 10:54pm by amanda

Chemistry- Buffers
a buffer is prepared by mixing .208 L of 0.452 M HCl and 0.5 L of 0.4 M sodium acetate. When the Ka= 1.8 x 10^-5 I figured out that the pH= 4.74 but then it asks how many grams of KOH must be added to the buffer to change the pH by .155 units?
Sunday, December 5, 2010 at 9:53pm by Mikey

Chemistry- Buffers
Show me how you obtained pH = 4.74. I can't get that. My answer looked more like 4.79.
Sunday, December 5, 2010 at 9:53pm by DrBob222

Chemistry
An industrial chemist studying bleaching and sterilizing prepares several hypochlorite buffers. Find the pH of the following buffers. (a) 0.090 M HClO and 0.090 M NaClO (b) 0.090 M HClO and 0.135 M NaClO (c) 0.135 M HClO and 0.090 M NaClO (d) One liter of the solution in part...
Monday, March 4, 2013 at 8:53pm by Edward

chemistry
1. Compare the effects of adding the strong acid & base to the pH of water vs. the acetate and phosphate buffers.
Wednesday, October 24, 2012 at 2:15pm by hi

biochemistry with more info that was needed
which buffer do I choose? There are instructions above the table does this have anything to do with my choice for the problem i am working out, or do I just pick whatever one I want and do the math? Above the table it states, Make two buffers starting with solid material, ...
Sunday, January 27, 2008 at 5:35pm by stew

Science- Chemistry
How many grams of sodium acetate( molar mass 82.03 g/mol) must me added to 1.00L of a 0.200M acetic acid solution to form a buffer of 4.20?Ka value for aceic acid is 1.8 x 10^-5. How do I go about finding the grams from the given information? http://www.chembuddy.com/?left=pH-...
Saturday, June 2, 2007 at 4:31pm by Catherine

chemistry
The Henderson-Hasselbalch equation for buffers is pH = pKa + log (base/acid) If you want (base) = (acid), then log base/acid is log 1 and that is zero; therefore, pH is pKa. Just look up the pKa for the acid of each pair and that will be the pH.
Sunday, October 9, 2011 at 1:43pm by DrBob222

Chemistry - buffers
Laborant got a task to make a buffer, which pH = 8.00. Which same concentration solutions and which ratio would you suggest him to mix?
Monday, March 26, 2012 at 2:39pm by Anonymous

Chemistry- Buffers
-log Ka = pKa which may or may not be = pH. Ka is a measure of how strong/weak the acid is.
Sunday, December 5, 2010 at 9:53pm by DrBob222

Chemistry, pH, Buffers
Is the 18.47 mL base used the amount to titrate to the equivalence point. Is the pH at the equivalence point 3.49 or is that some other point on the titration curve? I don't get a molar mass of 165.3 from the data above. Is there more data? I suspect so. Please type the entire...
Monday, April 2, 2012 at 11:44am by DrBob222

College Chemistry
Calculate the ratio of NaF to HF required to create a buffer with pH=3.95. Also, can you please explain in a nutshell the whole concept of buffers? Thanks!
Tuesday, March 23, 2010 at 10:44pm by Katie

buffers
thanks. so for this question is the pH 3.70?
Wednesday, March 3, 2010 at 10:55pm by Reen

chemistry - buffers
what mass of sodium acetate should be dissolved in 1.00L of acetic acid, 0.150M concentration, in order to produce a buffer with pH = 4.5?. Ka of CH3COOH = 1.8x10^-5
Monday, April 12, 2010 at 7:38pm by Reen

Chem Lab
Can the NH3/NH4Cl system be sued to prepare a buffer of a pH 9.5? why or why not? Can it prepare a buffer of pH 5? There were two buffers, 0.2 M and 0.1M.
Wednesday, April 11, 2012 at 11:21pm by Logan

Chemistry, pH, Buffers
Please help!! Given this data: mass of unknown acid 1.4671g Volume of NaOH used in titration 18.47mL Concentration of the NaOH used 0.2403M pH of the original acid solution 2.16 pH of the final acid solution 3.49 Show me how do I calculate the Ka of the unknown acid and the ...
Monday, April 2, 2012 at 11:44am by Krina

Chemistry, Buffers, pH
Hi could someone please help me in the next 5 minutes with this question: Given this data: mass of unknown acid 1.4671g Volume of NaOH used in titration 18.47mL Concentration of the NaOH used 0.2403M pH of the original acid solution 2.16 pH of the final acid solution 3.49 Show...
Friday, September 26, 2008 at 1:30am by janet

Chemistry (buffers)
Say, for example, that you had prepared a Buffer C, in which you mixed 8.203 g of sodium acetate, NaC2H3O2, with 100.0 mL of 1.0 M acetic acid. a. What would be the initial pH of Buffer C? HOW???????
Thursday, March 15, 2012 at 7:30pm by James

bio chemistry
calculate the PH of each of the following buffers prepared by placing in 1.0 L of solution 0.10 mol NH3 and 0.10 mol of NH4CL
Friday, March 2, 2012 at 11:11am by samar

buffers
I calculate 3.698 pH which rounds to 3.70. Yes. Very good.
Wednesday, March 3, 2010 at 10:55pm by DrBob222

Chemistry
I did an experiment on Buffers: In a polystyrene beaker, mix 20 ml of 0.1M Acetic acid ad 25 ml of 0.1 M sodium acetate and immediately measure the pH. Remove the electrode and add 5 ml of 0.1 M HCL to this buffer. Stir the solution and measure the pH. This is my data: Conc.of...
Thursday, July 16, 2009 at 3:36am by Saira

Chemistry- Buffers
Since Ka a measure of H+ ions, -log(Ka)= pH.. my assignment says that part is right, I just don't know what to do from there to get M -> moles -> grams
Sunday, December 5, 2010 at 9:53pm by Mikey

Chemistry - buffers
Two burettes are filled with solutions: one with 0,1OM CH3COOH solution, second with 0,15M CH3COONa. How many milliliters each solution will need to make 20mL of solution, which pH=4.85
Monday, March 26, 2012 at 2:43pm by Anonymous

biochemistry with more info that was needed
okay, let me just stick to the pre-lab question using the table. Here is the pre-lab question: Calculate the weight of the buffers you will use to make the buffers for part A for all the buffer possibilities listed under procedures in part A, stp i. In other words, how many ...
Sunday, January 27, 2008 at 5:35pm by stew

chemistry
A buffer is prepared by dissolving .0250 mol of sodium nitrite, NaNO2, in 250.0 mL of .0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer. My book does a poor job of explaining buffers and I'm really lost on the concept...
Sunday, April 29, 2007 at 7:30pm by Simpson

chemistry - buffers
Use the Henderson-Hasselbalch equation. pH = pKa + log (base/acid) Plug in pH needed, pKa for acetic acid, (HAc) for acid in the log term, and solve for base (acetate). That will be the concn of sodium acetate. For 1 L in the problem, that = moles and mols = grams/molar mass. ...
Monday, April 12, 2010 at 7:38pm by DrBob222

Chemistry- Acids and Buffers
Cyanic Acid is a weak acid HOCN + H2O <--> H3O+ +OCN- ka= 3.5*10^-4 a) if 2.5ml of 0.01 M cyanic acid solution is added to 25.0 ml of a formis acid buffer with ph = 3.70, what is the ratio of [OCN-]/[HOCN] in the resulting solution? b) determine the pH of a 0.500 M ...
Monday, April 9, 2012 at 4:21am by Tasneem

Chemistry
Describe how a buffer behaves. Your description should include an explanation of why the addition of NaOH to the HAc solution formed a buffer. What happens to the pH when a small quantity of a strong acid or base is added to a buffer solution? What happens to the pH of the ...
Thursday, March 14, 2013 at 2:20am by Terrell

Biochemistry
Dr. Bob222 is correct, you will need to add base to increase the pH of HEPES to 8, since the pKA of the solution is at 7.5. Remember, buffers have equal concentrations of its acid and conjugate base. Therefore, the pH of the solution is equal to the pKa.
Wednesday, January 30, 2013 at 9:49pm by Devron

chemistry
Disadvantage of using pH indicators for what? For titrations it is that not all indicators change at the equivalence point pH. If for determining the pH of a solution, it is because most pH indicators have a pH range of about 2 pH units which isn't very close if you want to ...
Wednesday, April 29, 2009 at 8:23pm by DrBob222

Chemistry
Classify each of the following solutions as acidic, basic, or neutral based on the pH value. (a) pH = 8.0 (b) pH = 7.0 (c) pH = 3.5 (d) pH = 6.1
Saturday, July 30, 2011 at 8:09pm by norma

Chemistry
Use the Henderson-Hasselbalch equation. That's what you use for buffers. pH = pKa + log (base)/(acid) The base is the K salt and the acid is propionic acid.
Thursday, March 21, 2013 at 9:20pm by DrBob222

chemistry
First, hydrogen peroxide is always in a solution of water. Adding NH3 to that forms hydrogen peroxide and ammonium hydroxide. Now, other things come into play. Normally, there are stabilizers and pH adjusting buffers in the peroxide, these wont do much except let the peroxide ...
Thursday, October 2, 2008 at 11:23pm by bobpursley

Chemistry
Which solution below has the highest concentration of hydronium ions? pH = 9.82 pH = 12.6 pH = 7.93 pH = 3.21 pH = 7.00
Tuesday, March 19, 2013 at 7:26pm by DrewS

Chemistry- Acids and Buffers
HOCN ==> H^+ + OCN^- Ka = (H^+)(OCN^-)/(HOCN) For a. The formic acid buffer is pH 3.70 which is H^+ = 2E-4 Ka = (H^+)(OCN^-)/(HOCN) Rearrange to (OCN^-)/(HOCN) = Ka/(H^+) Substitute Ka/(H^+) and you have it. ........HOCN ==> H^+ + OCN^- initial..0.5......0......0 change...
Monday, April 9, 2012 at 4:21am by DrBob222

buffers
9.00mL of 1.10M CH3COOH and 1.00mL of 0.900M CH3COO- what is the pH?
Wednesday, March 3, 2010 at 10:55pm by Reen

Chemistry
3 buffers in the human body and what are their conjugate acid-base pairs? I have Bicarbonate Buffer, Phosphate/Ammonia Buffer, and Protein Buffers, where my confusion lies in what would be there conjugate acid base pairs.......
Saturday, November 12, 2011 at 4:21pm by Mandie

chemistry
I have already posted this and never got a response, please help. here is my data from lab: Buffer1: HPO4- weight 3.412g; original pH Buffer 2: HEPES wt: 1.090g original pH 10.08 buffer1: pH of 0.1M: 7.5; pH of 0.01: 7.72; pH of 0.001M: 7.87 buffer2: PH of 0.1M: 7.5 ph of 0.01...
Sunday, February 3, 2008 at 2:49pm by student

Chemistry
Okay, so based on the chart in my book I was able to determine the following. pH=(unknown) pKa=7.2 of Phosphoric Acid (2) A-=.5M of Na2HPO4 HA=.3M H2PO4- pH= 7.2 + log(.5/.3) pH=7.2+log(1.6667) pH=7.2+0.5108 So, the pH of this solution is: pH=7.7108 Correct?
Wednesday, July 6, 2011 at 11:13am by Shaun

Chemistry - buffers
If that's all of it then your prof didn't give very good directions. I have no idea which acid he/she has in mind so I'll fly blind. I looked at the Ka values and picked HOCl. With pH = 8 for a buffer I might pick HOCl for the acid with Ka = 3.0E-8 (you need to see what that ...
Monday, March 26, 2012 at 2:39pm by DrBob222

Analytical chemistry
What is a pH of 20 mL of 0.08 M NH3 added to 40 mL of 0.04 M HCl? NH3 + HCl = NH4+ + Cl- c(NH3)=(0.02L * 0.08M)/0.06L= 0.02667 M c(HCl)=(0.04L * 0.04M)/0.06L= 0.02667 M c(NH4+)=c(HCl) Kb=[NH4+][OH-]/[NH3] Kb=1.76*10^(-5) So i tried to calculate it like this: Kb=[OH-] pOH=4....
Monday, September 2, 2013 at 8:11am by Gloria

Chemistry
A = pH of 8. 1,000 times means difference in pH of 3. If it is more H^+, then pH = 5 for the new solution. Is that acid or basic. pH<7 = acid pH=7 = neutral pH>7 = basic
Monday, November 14, 2011 at 3:56pm by DrBob222

chemistry (buffers)
Buffers are combinations of a weak acid and a weak base, not a weak acid and a strong base.
Monday, September 1, 2008 at 3:15am by GK

Chemistry -buffers.
The pH of an arterial blood sample is 7.15. upon acidification of 10 ml of the plasma 5.91ml of CO2 is produced at standard temperature and presure. Calculate-a) total CO2 in the specimen b)the individual concentration of disolved CO2(H2CO3) and HCO3- c)The partial pressure of...
Sunday, November 6, 2011 at 12:14am by Maria

Chemistry
Buffers- Common Ion effect IS this Correct Calculate the pH of a aqueous solution containing 0.15 M HNO2 and 0.20 M NaNO2 (aq). The Ka of nitrous acid is 4.0*10^-4. HNO2 + H20 <--> NaNO2- + H30^+ Inital 0.15 0.20 X Final 0.15 0.20 Ka= [H30+][NaNO2]/ [HNO2] 4.0*10^-4 = [...
Tuesday, August 11, 2009 at 8:17am by Saira

chemistry buffers
What molar ratio of HPO4 2- to H2PO4 - in solution would produce a pH of 7.0? Phosphoric acid (H3PO4), a triprotonic acid, has pKa values: 2.14, 6.86, and 12.4. Only one of the pKa values is relevant here. how do i know which pka value to use.. please explain
Sunday, September 9, 2012 at 4:28pm by ron

chemistry
pH pure H2O = 7 (H^+) = (OH^-) = 1E-7M acid pH < 7 base pH > 7 neutral pH = 7
Sunday, April 21, 2013 at 12:44pm by DrBob222

chemistry
which solution has the highest concentration of hydroxide ions? a ph=7.93 b ph=12.59 c ph=7.00 d ph=9.82 e ph=3.21 i know the answer is 7 but why is it seven? would it be different if it said hydronium ions?
Saturday, December 11, 2010 at 1:07pm by jessie

chemistry
No, that isn't correct. The more acidic the solution, the lower the pH. pH <7 = acid pH = 7 neutral pH >7 = basic
Tuesday, November 8, 2011 at 6:27am by DrBob222

chem 2
Please don't change screen names. Buffers are most effective when the pKa is in the range of desired pH; and that means base/acid = 1 So you want to pick the NaC2H3O2 concn that gives the value closest to b/a = 1.
Saturday, March 3, 2012 at 1:55pm by DrBob222

Chemistry
I actually posted this up before and Gk helped out but i don't understand the steps what do i enter for the pka for the first one? __________________________________________ I did an experiment on Buffers: In a polystyrene beaker, mix 20 ml of 0.1M Acetic acid ad 25 ml of 0.1 ...
Sunday, July 19, 2009 at 7:24am by Saira

Chemistry
How many moles of NaOH must be added to 1.0 L of 2.2 M HF to produce a solution buffered at each pH? (a) pH = pKa (b) pH = 4.24 (c) pH = 4.60
Wednesday, March 13, 2013 at 2:48am by Margaret

Chemistry
thank Dr.Bob222 I see you got the same answer I did. I got one more I need help with if you can help me please Classify each of the following solutions as acidic, basic, or neutral based on the pH value. (a) pH = 8.0 (b) pH = 7.0 (c) pH = 3.5 (d) pH = 6.1
Saturday, July 30, 2011 at 5:37pm by norma

Chemistry
How will the addition of sodium acetate to an acetic acid solution affect the pH? A. solution becomes hotter B. It will lower the pH C. It will raise the pH D. pH will not change E. pH cannot be measured I selected answer D and got it wrong. I don't understand why...
Sunday, March 10, 2013 at 12:18pm by Lisa

AP Chemistry
Refer to your post below. pH = -log(H^+). Substitute and solve for (H^+). pH<7 = acid pH = 7 = neutral pH >7 = basic.
Wednesday, January 9, 2013 at 10:11pm by DrBob222

chemistry
What is the net charge on Phe-Asp at each pH? a. pH 1 b. pH 7 c. pH 14
Thursday, April 26, 2012 at 10:46pm by krystal

Chemistry
a. pH = -log(H^+) pH = -log(7E-4) pH = -(-3.15) pH = 3.15 b. pH + pOH = pKw = 14 pH + 6 = 14 pH = 8 The problems asks for (H^+); therefore, pH = -log(H^+) 8 = -log(H^+) -8 = log(H^+) (H^+) = 1E-8
Tuesday, April 30, 2013 at 11:21pm by DrBob222

chemistry
Perhaps this will help. http://www.chemcollective.org/buffers/buffers5.php
Monday, January 30, 2012 at 6:04pm by DrBob222

Chemistry
Calculate the molar hydroxide ion concentration of each of the following solutions given the pH: pH=0.90 AND pH=1.62 I know to covert from ph to hydroxide but i'm having a problem going from hydroxide to ph..can someone please help me..thanks
Thursday, May 5, 2011 at 12:38pm by Renee

Chemistry
You KNOW #1 and #3 are buffers.
Sunday, April 10, 2011 at 7:16pm by DrBob222

Chemistry-pH
If it's a liquid, I would use a pH meter. A colored sample doesn't necessarily negate measuring the pH with a piece of pH paper (litmus, for example) if the measurement doesn't need to be highly accurate.
Tuesday, January 25, 2011 at 5:12am by DrBob222

E.M.U
For the same solution components as in part (f), buffers are prepared with a total concentration of NH3 + NH4Cl = 0.10 M. The pH values are 8.0, 8.5, 9.0, 9.5, 10.0, 10.5, and 11.0. Find the molar solubility of CdS in these solutions
Wednesday, March 26, 2014 at 4:26pm by k.sina

organic chemistry
for each of the following compounds, draw the form in which it will predominate at ph=3, ph=6, ph=10, and ph=14. a)CH3COOH b)CH3CH2NH3 c) CF3CH2OH please explain how to get answers. my book does not give clear examples.
Thursday, May 30, 2013 at 8:26am by julia

Chemistry 130
pH = -log[H+] The above relationship can also be expressed as: [H+] = 10^(-pH) or [H+] = 1 / 10^(pH) That shows the hydrogen ion concentration is inversely proportional to the pH.
Tuesday, October 13, 2009 at 10:53am by GK

Chemistry
pH = -log(H^+) pH = -log(2) = -(0.301) = -0.301 pH<7 acidic pH = 7 neutral pH>7 basic
Tuesday, May 10, 2011 at 3:48pm by DrBob222

Chemistry
Here is a site that explains what pH is all about and gives a somewhat lengthy explanation of pH and the pH of common chemicals. It goes on to say that there are many factors that control the pH in lakes and that the pH varies with season as well as during the daylight and ...
Monday, May 12, 2008 at 11:48am by DrBob222

Chemistry
Sodium methanoate, NaHCOO, and methanoic acid, HCOOH, can be used to make a buffer solution. Explain how this combination resists changes in pH when small amounts of acid or base are added. Buffers kind of confuse me and I'm not sure how to start this. Can someone help me to ...
Thursday, April 4, 2013 at 4:37pm by a Canadian

Chemistry
I made a couple of mistakes 1: Equation is: pH = pKa + log([A-]/[HA] Notice addition instead of subtraction 2: Change in pH: pH = 4.202 + log(.0096/.0104) pH = 4.167
Thursday, November 1, 2012 at 1:00pm by Anonymous

Chemistry
Select the statements that correctly describe buffers.? 1) The pH of a buffer solution does not change significantly when any amount of a strong acid is added. 2) The Ka of a buffer does not change when any amount of an acid is added to the buffer solution. 3) The pH of a ...
Monday, September 23, 2013 at 11:06pm by Aria

Chemistry
I am having trouble with how to approach this problem. I have the solution but can't figure out how to get it. How many moles of NaOH must be added to 1.0 L of 2.0M HC2H3O2 to produce a solution buffered at each pH? a) pH=pKa b)pH=4 c)ph=5
Monday, April 12, 2010 at 6:42pm by Larry

chemistry
I am having trouble with how to approach this problem. I have the solution but can't figure out how to get it. How many moles of NaOH must be added to 1.0 L of 2.0M HC2H3O2 to produce a solution buffered at each pH? a) pH=pKa b)pH=4 c)ph=5
Monday, April 12, 2010 at 9:18pm by heather

science(chem)
I found the other site. Here it is. http://www.haverford.edu/chem/Scarrow/GenChem/acidbase/buffer_prep.html The usual biochemistry buffers means one thing and analytical chemists express buffers another way (or I may be out of touch with the new day thinking). At any rate, a 0...
Sunday, September 21, 2008 at 11:28pm by DrBob222

Chemistry
I just did a lab on Acids and Bases and I am having trouble with the lab questions I was given to complete. Concentration of NaOH: 0.09999 M Volume of NaOH: 3.25 mL # moles of NaOH: 0.325 moles Initial Concentration of Weak Acid: ? (How do we calculate this) Part 2: Hydrolysis...
Sunday, March 29, 2009 at 1:53pm by Lalu

Chemistry
How many moles of NaOH must be added to 1.0 L of 1.4 M HC2H3O2 to produce a solution buffered at each pH? (a) pH = pKa mol (b) pH = 3.07 mol (c) pH = 5.15 mol
Sunday, December 5, 2010 at 3:22pm by justin

Chemistry.
pH C ( dark green) pH : 8 d ( purple) pH : 3 Suppose u mix togather equal amounts of the solutions that produced the results of strip C and strip D , then test the pH of this new solution. What colo will the indicator paper be ? Explain.
Saturday, February 23, 2013 at 10:43am by Mia

Chemistry
Consider a solution that contains both C6H5NH2 and C6H5NH3+. Calculate the ratio [C6H5NH2]/[C6H5NH3+] if the solution has the following pH values. (Assume that the solution is at 25C.) (a) pH = 4.70 (b) pH = 5.26 (c) pH = 5.42 (d) pH = 4.96
Wednesday, March 13, 2013 at 2:47am by Margaret

Steph
Buffers work by converting _____ to ____.
Tuesday, November 1, 2011 at 10:38pm by Chemistry

Chemistry
Second thought I just don't understand what to do. pH= pKa + log [NH3]/[NH4NO3] pH= -l log ? + log (0.005/?) pH= ? pH= ?
Friday, November 11, 2011 at 8:45pm by Monique

Chemistry
Calculate the molar hydroxide ion concentration of each of the following solutions given the pH: pH=0.90 AND pH=1.62 I know to covert from ph to hydroxide but i'm having a problem going from hydroxide to ph..can someone please help me..thanks can someone please answer my ...
Thursday, May 5, 2011 at 12:38pm by Renee

chemistry
How much 6M HNO3 will be required to decrease the pH of 5000L solution of pH=9.6 to pH=3?
Friday, January 4, 2013 at 5:45am by vidya

chemistry
A distribution curve shows how the fractions of non ionized acid and its conjugate base vary as a function of Ph. The curves of the plot of [CH3COOH] vs. Ph and [CH3COO-] vs. Ph will intersect at a Ph of what? I need to show work
Sunday, April 22, 2012 at 1:30pm by court

chemistry
I assume you want the pH of the solution. pH = pKa + log(base)/(acid) Substitute and solve or pH.
Wednesday, October 24, 2012 at 8:20pm by DrBob222

chemistry
acetic acid: 0.1 M 30ml hydrochloric acid 0.1 M 5 ml sodium hydroxide 0.1 M 15 ml Buffer + 5ml of: 1.91 ph ph (measured): 4:52 ph HOW DO I CALCULATE PH(CALCULATED)? AND ALSO IT SAYS SHOW YOUR CALCULATION FOR THE PH OF THE BUFFER BEFIRE AND AFTER THE ADDITION OF HCL? COULD YOU ...
Saturday, July 14, 2012 at 6:28pm by fenerbahce

chemistry
pH = pKa + log ([A-]/[HA]) pH = pKa + log ([C2H3O2-] / [HC2H3O2]) pH = -log (1.8 x 10-5) + log (0.50 M / 0.20 M) pH = -log (1.8 x 10-5) + log (2.5) pH = 4.7 + 0.40 pH = 5.1 I used this example And I still got it wrong it should have been 4.75 + 0.12 = 4.87 or do I use just 4.7...
Friday, November 11, 2011 at 8:02pm by Monique

chemistry
pH of 3 is acidic. pH of 10.5 is basic. The water is pH of 7 and neutral.
Saturday, June 25, 2011 at 9:48pm by DrBob222

chemistry
1E-5 H^+ = pH = 5 2E-4 H^+ = pH = 3.7 pH + pOH = pKw = 14
Sunday, July 10, 2011 at 1:38pm by DrBob222

Chemistry
pH = 7 is neutral pH<7 = acidic pH>7 = basic
Saturday, July 30, 2011 at 5:37pm by DrBob222

chemistry
pH = 7 = neutral pH < 7 = acidic pH > 7 = basic
Monday, December 5, 2011 at 2:19pm by DrBob222

Chemistry
Let's see. If we dilute 0.1(pH = 1) to 0.01 (pH = 2), is that a decrease in pH? :-) I think it can't be a, b, or c.
Monday, May 20, 2013 at 2:58pm by DrBob222

chemistry
Calculate the solubility of Mn(OH)2 in grams per liter when buffered at each of the following. (a) pH 7.7 (b) pH 9.6 (c) pH 11.3
Wednesday, March 27, 2013 at 10:35am by hannah

Chemistry (Acids and Bases)
I just did a lab on Acids and Bases and I am having trouble with the lab questions I was given to complete. Concentration of NaOH: 0.09999 M Volume of NaOH: 3.25 mL # moles of NaOH: 0.325 moles Initial Concentration of Weak Acid: ? (How do we calculate this) Part 2: Hydrolysis...
Sunday, March 29, 2009 at 1:54pm by Lalu

Chemistry - buffers
Thank you very much for the help! Now I see what should I do.
Monday, March 26, 2012 at 2:39pm by Anonymous

Chemistry
Both of these are buffers. Use the Henderson-Hasselbalch equation.
Tuesday, May 1, 2012 at 5:02pm by DrBob222

AP CHEMISTRY
Calculate the solubility of Mn(OH)2 in GRAMS PER LITER when buffered at each of the following. a)pH 7.4 b)pH 9.2 c) pH 11.5
Saturday, March 10, 2012 at 4:01pm by JIM

AP CHEMISTRY
Calculate the solubility of Mn(OH)2 in GRAMS PER LITER when buffered at each of the following. a)pH 7.4 b)pH 9.2 c) pH 11.5
Saturday, March 10, 2012 at 4:14pm by fernatesfsdf

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